Short Chemistry About Ionic Packet For Lab Chemistry For Ionic Atoms Ans Duck Chemistry Assignment

1876 words - 8 pages

Chemical Bonds – Ionic Bonds
1. Identify the Number of Valance Electrons and Draw the Lewis Dot Structure
Notes: Scientists use Lewis Dot Structures to show the valance electrons of an element as dots. Since bonding involves the valance shell electrons only, it is only necessary to illustrate those outer electrons.
Element
Bohr Diagram
Group Number (PT)
# of Valance Electrons
Lewis Dot Structure
Calcium
Carbon
Hydrogen
Helium
Oxygen
Fluorine
Neon
Sodium
Aluminum
Determining the Ionic Charge
Element
Property
Before Making an Octet
After Making an Octet
Li
electron config
# protons
#electrons
charge
Bohr Diagram
Lewis Dot Structure
Be
electron config
# protons
#electrons
charge
Bohr Diagram
Lewis Dot Structure
B
electron config
# protons
#electrons
charge
Bohr Diagram
Lewis Dot Structure
Skip Carbon
N
electron config
# protons
#electrons
charge
Bohr Diagram
Lewis Dot Structure
O
electron config
# protons
#electrons
charge
Bohr Diagram
Lewis Dot Structure
F
electron config
# protons
#electrons
charge
Bohr Diagram
Lewis Dot Structure
Ne
electron config
# protons
#electrons
charge
Bohr Diagram
Lewis Dot
Making Ions – Ionic Bonds are made of Ions. A strong understanding of Ions is needed.
Notes: Remember that Metals tend to lose their electrons, falling back to their inner octet, becoming smaller, forming positive “cations”. Nonmetals tend to gain electrons, filling up their current energy levels, becoming larger, forming negative “anions”. Complete the chart below.
Element
Lewis Dot
# of Valance e-
Gain/Lose ___ e-
Valance Charge
Na
1
L 1
+1
Be
Cl
S
Al
Ne
K
N
O
Ca
P
B
Mg
Lewis Dot, Formula Unit & Naming Practice Sheet
Notes:
1. An ionic bond is an attraction of a cation for an anion resulting from the transfer of electrons. Remember, the smaller nonmetals are more electronegative and pull the electrons close, away from the larger, less electronegative metals.
2. When naming ionic compounds, the Metal is named first, followed by the nonmetal with an –ide ending. Ex. Sodium Fluorine becomes Sodium Fluoride.
3. Formula Unit: Lowest whole number ratio of elements in the compound. Ex. Ca3N2
1. Draw the Lewis Structure for Mg & Cl
Formula Unit: _________
Name of Compound:
2. Draw the Lewis Structure for Mg & S
Formula Unit: _________
Name of Compound:
3. Draw the Lewis Structure for K & F
Formula Unit: _________
Name of Compound:
4. Draw the Lewis Structure for K & O
Formula Unit: _________
Name of Compound:
5. Draw the Lewis Structure for Be & N
Formula Unit: _________
Name of Compound:
6. Draw the Lewis Structure for Ca & P
Formula Unit: _________
Name of Compound:
7. Draw the Lewis Structure for Al & F
Formula Unit: _________
Name of Compound:
8. Draw the Lewis Structure for Ca & I
Formula Unit: _________
Name of Compound:
9. Draw the Lewis Structure for Rb & O
Formula Unit: _________
Name of Compound:
10. Draw the Lewis Structure for Sr & F
Formula Unit: _________
Name of Compound:
11. Draw the Lewis Structure for Al & Cl
Formula...

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